EXAM REVIEW
Covalent bonding
Ionic bonding
Metallic Bonding
H is in group 1. What other group could it fit into based on how it bonds?
What group on periodic table has most reactive non-metals?
What group on the periodic table has most reactive metals?
2 gainers…what type of bond?
What does the zigzag line separate on the periodic table?
Most elements on the table are…………… & ………………………
What is the difference between a group and family?
What do every element in group 13 have in common? Group 14? Group 15?
What do elements in the same period have in common?
What is a diatomic element? What does periodic mean?
What is unique about group 18, the Noble Gas family?
Metals tend to gain/lose (circle one) to bond.
Non-metals tend to gain/lose (circle one) to bond.
Ions are? A -2 ion has 8 protons, how many electrons?
A +3 ion has 13 protons, how many electrons?
How does an atom become a negative ion?
How does an atom become a positive ion?
What type of bond makes materials ductile &/or malleable?
For the next 7--- label as metallic bond OR covalent bond OR ionic bond.
1. Transfer electrons_________________
2. Metal reacts w/ non-metal____________________
3. Attraction b/t nuclei & shared e-________________4. Conduct heat & electricity_____________________
5. Ions(charged particles) formed_________________6. “Sea of e-“ formed___________________________
7. Diatomic elements___________________________
List 2 things that are not matter.
Label each of the following as either a phys change or a chem. Change: rusting, burning, freezing, tarnishing
When elements combine chemically do they lose or keep their own properties?
Which material vibrates in place? Solids/liquids/gases
Are there empty spaces between molecules? Explain.
As mass goes up, what else goes up?
What property changes when you go to the moon? Why?
What is gravity? What 2 factors determine gravity?
What is sublimation & give 3 examples.
What is the difference b/t chemical change & chemical reaction?
Define hetero- & give example of heterogeneous matter. Define suspension & give example.
An example of colloid, solution, compound, element.
Circle the compounds: N2
H2O
Fe
CO
Co
Which of the above is a diatomic element?
Put 2or more things together (not chemically) what is it?
-ology means? -geneous means? Density of water is?
Charles Law decrease temperature = ??? increase temp=??
Parts of a mixture ___________most of their own properties.
Mass 12g and volume 4 ml: What is the density? Float/sink?
Water on the outside of a pop bottle in summer, explain.
Gas volume is 30 cm3 pressure is 5ppi. Pressure increases to 10ppi. What is new volume? Whose law?
Define, describe tools and units for the following terms: mass, weight, volume, density, temperature.
Describe reactants and products in a chemical equation.
Describe the arrangement, motion & energy of solids, liquids and gases. Are ice & water the same thing? Explain.
Location, charge & mass of the following particles: electron, neutron, proton
The same element always has the same number of____
C-15 atomic number 6: How many neutrons, protons, electrons?
What are valence electrons?
What particle defines the element?
Atomos, Latin for_________________________
U-235, U-236 How are they similar & how are they different? Number of protons, electrons & neutrons for each?
Nitrogen has an atomic number of 7 and a mass number of 16. How many protons, neutrons, & electrons?
WRITING FORMULA SHEET NECESSARY!
Circle the coefficient.
3 Na(ClO3)4
What is the subscript for sodium?
Underline the subscript for oxygen.
What is the name of the compound. How many atoms of sodium are present?
Cl?
O?
2 KCl --- What is the name of this substance? What is the coefficient?
Write the formula for Iron (II) oxide.
Write the formula for Iron (III) oxide.
Write the name for CuO.
Write the name for Cu2O.
1. Which of the following is a balanced equation?
a.
Na +
Cl2 ----- 2 NaCl
c.
2 NaCl + O2 -- 2 NaO
b.
+ Cl2
d.
2 NaCl ------- Na + Cl2
2 NaCl + H2O ------ NaO + 2 HCl
2. How many carbon atoms are in this molecule of glucose?
C6H12O6 How many H?
O?
3. Which of the following substances can be found in every living thing?
4. What is/are the product(s) in this equation,
Na +
Cl2 ----- NaCl
5. Write out the correct balanced chemical equation for photosynthesis?
6. Is photosynthesis exothermic or endothermic? Why?
7. What is the opposite of photosynthesis? ___________________________________
Balance:
O2 + C6H12O6 --- CO2 + H2O
(+ energy released so it is _______-thermic )
8. The Law of Conservation of Matter is states that matter cannot be______________________ OR
____________________ which is why equations must be________________________________.
9. How many oxygen atoms are present in the REACTANT side of the following chemical
How many on the product side?
4Fe + 3O2 -- Fe2O3
equation?
Is this equation balanced?
1. What are the products formed when HCl reacts with NaOH in a double replacement, neutralization reaction?
a. NaH & ClOH
b. H2 & NaOCl
c. Cl2 & NaH2O2
d. NaCl & H2O
2. The subscript in the chemical formula H2O tells you there are two:
a. atoms of hydrogen in the molecule
b. electrons of the hydrogen atom in the molecule
c. elements in the molecule
d. atoms of oxygen in the molecule
3. The coefficient 2 in 2CO2 means that there are
a. two oxygen atoms and one carbon atom present.
b. two oxygen atoms present.
c. two carbon atoms and two oxygen atoms present.
d. two carbon dioxide molecules present.
Use the reaction types below to match the reaction descriptions questions belo.
a. decomposition
b. double replacement
c. single replacement
d. synthesis
4. Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen.
5. Water can be broken down to form hydrogen and oxygen.
6. Magnesium reacts with oxygen in the air to form magnesium oxide.
7. Sodium fluoride and silver chloride are formed from the reaction of sodium chloride with silver chloride.
8. Which of the following statements about chemical reactions is NOT true?
a. Exothermic reactions release energy.
b. Energy can be stored in molecules.
c. Endothermic reactions release energy.
d. All chemical reaction requires some energy to get started.
9. Name 2 endothermic reactions? Name 2 exothermic reactions?